뒤로Electronic Structure of Atoms - General Chemistry
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이 집합의 용어 (27)
Wavelength (λ) is the distance between corresponding points on adjacent waves in electromagnetic radiation.
Frequency (ν) is the number of complete waves passing a given point per unit time, typically per second.
For waves traveling at the same velocity, the longer the wavelength, the smaller the frequency.
The speed of light is \(3.00 \times 10^{8}~m/s\). It relates to wavelength and frequency by \(c = \lambda \nu\).
1) Blackbody radiation, 2) Photoelectric effect, 3) Emission spectra of excited gas atoms.
Quanta are discrete packets of energy that energy is emitted or absorbed in, rather than continuous waves.
\(E = h \nu\), where h is Planck's constant \(6.626 \times 10^{-34}~J\cdot s\).
Continuous spectra show all wavelengths (like a rainbow), while line spectra show discrete wavelengths unique to each element.
Electrons orbit the nucleus in specific allowed orbits with quantized energies; energy is emitted or absorbed when electrons change orbits.
The ground state is the lowest energy state of an electron; any higher energy state is an excited state.
ΔE < 0 means photon is emitted (energy released); ΔE > 0 means photon is absorbed (energy gained).
It only accurately describes hydrogen; it assumes electrons do not spiral into the nucleus and treats electron motion as circular, not wave-like.
Matter exhibits wave properties, with wavelength related to momentum by \(\lambda = \frac{h}{mv}\).
The more precisely a particle's momentum is known, the less precisely its position can be known, expressed as \(\Delta x \Delta p \geq \frac{h}{4\pi}\).
It mathematically describes electrons as wave functions, giving probabilities of electron locations rather than fixed orbits.
Quantum numbers describe the energy, shape, and orientation of atomic orbitals where electrons are likely found.
n describes the energy level of an orbital and takes integer values ≥ 1.
l defines the shape of the orbital, with values from 0 to n-1, corresponding to s, p, d, f orbitals.
ml describes the orientation of an orbital in space, with values from -l to +l.
ms describes the electron's spin, with allowed values of +1/2 or -1/2.
No two electrons in the same atom can have the same set of four quantum numbers (n, l, ml, ms).
It is the arrangement of electrons in an atom's orbitals, showing energy levels, orbital types, and electron counts.
Electrons fill degenerate orbitals singly first, with parallel spins, to maximize total spin.
Valence electrons are in the outermost shell; core electrons are in filled inner shells.
Using the noble gas symbol for core electrons in brackets, followed by valence electron configuration.
Electrons may occupy orbitals to half-fill or fully fill d or f subshells for extra stability, deviating from expected order.
Blocks correspond to orbital types: s, p, d, f; electron filling follows increasing energy order reflected in the table.